A sample of an unknown compound with a mass of 0.847 g has the following composition: 50.51 percent fluorine?

Question

and 49.49 percent iron. When this compund is decomposed into its elements, what mass of each element would be recovered?

Answer 1

0.847 x .5051 = 0.428 g Fluorine
0.847 x .4949 = 0.419 g Fe

Answer 2

If opportunities are given, anticipate you have a hundred g of the compound, changing each % image with "g". on occasion, g contraptions are already given. a million. Convert each mass into moles. (38.40 4 g C)(a million mol/12.0 g) = 3.203 mol C (4.839 g H)(a million mol/a million.008 g) = 4.801 mol H (fifty six.seventy 3 g Cl)(a million mol/35.40 5 g) = a million.600 mol Cl 2. Divide each mole quantity with the aid of the smallest quantity (a million.600) and get: 2.00 mol C 3.00 mol H a million.00 mol Cl The empirical formulation may be C2H3Cl, which might have a molar mass of sixty two.5 g/mol To get the molar mass stated in the subject, you ought to double the empirical formulation: The molecular formulation may be C4H6Cl2, which has a molar mass of 123 g/mol

Answer 3

If you can't figure this one out, it's time to pack up and go home. What part of mass and percent can't you understand?